chem 1201 HW Ch. 6 p 2
Indicate how many unpaired electrons each atom has. Drag the appropriate items to their respective bins
0 unpaired electrons: Ca 1 unpaired electron: Br, Y, Lu 2 unpaired electrons: Sn 3 unpaired electrons: V 4 unpaired electrons: none 5 unpaired electrons: none
Complete an orbital diagram for boron. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all.
1s: 2 arrows 2s: 2 arrows 2p: 1 arrow in the first orbital (leave the rest empty)
Electron configurations are a shorthand form of an orbital diagram, describing which orbitals are occupied for a given element. For example, 1s22s22p1 is the electron configuration of boron. Use this tool to generate the electron configuration of arsenic (As).
1s: 2 arrows 2s: 2 arrows 2p: 2 arrows in 3 orbitals 3s: 2 arrows 3p: 2 arrows in 3 orbitals 4s: 2 arrows 3d: 2 arrows in 5 orbitals 4p: 1 arrow in 3 orbitals [Ar]4s^2 3d^10 4p^3
Complete an orbital diagram for scandium (Sc). Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all.
1s: 2 arrows 2s: 2 arrows 2p: 2 arrows in all 3 orbitals 3s: 2 arrows 3p: 2 arrows in all 3 orbitals 4s: 2 arrows 3d: 1 arrow in the first orbital (leave the rest empty)
The probability of finding an electron anywhere in a spherical radius of r is called the radial probability distribution. The shape of the plot depends on the principal quantum number (n) and the azimuthal quantum number (ℓ) for an orbital. As n increases for each value of ℓ, the number of nodes in the plot increases by one. To understand the radial distribution function for different orbitals, match the orbital that corresponds to the radial distribution function shown in each plot. Identify the radial distribution functions by dragging the appropriate orbitals to their respective targets.
2p 3p 3d
Which one of the following represents an impossible set of quantum numbers for an electron in an atom? (arranged as n, l, m l , and ms)
4, 3, 0, 0
Identify which sets of quantum numbers are valid for an electron. Each set is ordered (n,ℓ,mℓ,ms). Check all that apply.
4, 3, 1, -1/2 3, 2, -2, 1/2 1, 0, 0, -1/2 3, 0, 0, 1/2 2, 1, -1, -1/2
A three-dimensional plot of the wave function squared (ψ2) produces a diagram showing the probability density for an electron as a function of distance from the nucleus. These solutions are called orbitals. Three solutions to ψ2 are plotted here. Identify the orbital shown in each plot.
A p orbital (dumbbell) A s orbital (sphere) A d orbital (double dumbbell)
Classify each orbital diagram for ground-state electron configurations by the rule or principle it violates. Drag the appropriate items to their respective bins.
Aufbau violation: arrows in 3p when 3s isn't completed arrows in 3d when 4s doesn't come before it Hund violation: arrow down in 4d (it should be facing upwards) two arrows in first 3p orbital (single arrows should be spread out facing upwards in each subshell before pairing occurs) Pauli violation: arrows facing the same direction in 2s (paired electrons should always face the opposite direction)
Using equation E=(hcRH)(1n2)=(−2.18×10−18J)(1n2), calculate the energy of an electron in the hydrogen atom when n=2.
E2 = −5.45×10−19 J
Using equation E=(hcRH)(1n2)=(−2.18×10−18J)(1n2), calculate the energy of an electron in the hydrogen atom when n= 5.
E5 = −8.72×10−20 J
Identify the sets of quantum numbers that describe all the electrons in the ground state of a neutral beryllium atom, Be. Each set is ordered (n,ℓ,mℓ,ms).
Electrons in Be: 2,0,0,1/2 1,0,0,-1/2 1,0,0,1/2 2,0,0,-1/2 Electrons not in Be 2,1,0,1/2 2,1,0,-1/2 2,1,-1,-1/2 2,1,-1,1/2
The following sets of quantum numbers, listed in the order n, ℓ, mℓ, and ms, were written for the last electrons added to an atom. Identify which sets are valid and classify the others by the rule or principle that is violated. Drag the appropriate items to their respective bins.
Pauli violation: 5 2 -1 +1/2 5 2 0 +1/2 5 2 +1 +1/2 5 2 0 +1/2 5 2 +2 +1/2 Other violation: 3 1 -1 +1/2 3 1 0 +1/2 3 -1 +1 +1/2 valid: the other two sets
The probability of finding an electron at a point in an atom is referred to as the probability density (ψ2). The spatial distribution of these densities can be derived from the radial wave function R(r) and angular wave function Y(θ,ϕ), then solving the Schrödinger equation for a specific set of quantum numbers. Which of the following statements about nodes and probability density are accurate?
The 3p orbitals have two nodes. The 4f orbitals have three nodes. The probability of finding an electron at the center of a p orbital is zero.
1s^2 2s^2 2p^6 3s^2 3d^5
The orbitals are not filled in order of increasing energy.
1s^2 2s^2 3s^2
The orbitals are not filled in order of increasing energy.
[Xe]6s^2 5d^4
The orbitals are not filled in order of increasing energy.
Write the condensed electron configurations for the Ca atom. Express your answer in condensed form as a series of orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.
[Ar]4s^2
Write the condensed electron configurations for the Br atom. Express your answer in condensed form as a series of orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.
[Ar]4s^23d^104p^5
Write the condensed electron configurations for the V atom. Express your answer in condensed form as a series of orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.
[Ar]4s^23d^3
Write the condensed electron configurations for the Sn atom. Express your answer in condensed form as a series of orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.
[Kr]5s^2 4d^10 5p^2
Write the condensed electron configurations for the Y atom.
[Kr]5s^24d^1
Write the condensed electron configurations for the Lu atom.
[Xe]6s^24f^145d^1
What is the label for the orbital shown here that indicates the type of orbital and its orientation in space? Express your answer using appropriate letters (e.g., px). Do not include the energy level n.
d_yz
Part A Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen.
energy is emitted: from an orbit of radius = 4.76 Å to one of radius 0.529 Å energy is absorbed: from the n=6 to the n=9 state from the n=2 to the n=5 state
Identify the general outer electron configuration for each group of elements shown in this periodic table outline.
it wouldn't hurt if you could just look at a periodic table... Group 1 (H and below): ns^1 Sc, Y: ns^2(n-1)d^1 Ne, Ar: ns^2np^6 Se, Te: ns^2(n-1)d^10np^4 Tl, Nh: ns^2(n-2)f^14(n-1)d^10np^1
Give the numerical value of l corresponding to 2s.
l = 0
Give the numerical value of l corresponding to 3p.
l = 1
Give the numerical value of l corresponding to 5d.
l = 2
Give the numerical value of l corresponding to 4f.
l = 3
Place the following transitions of the hydrogen atom in order from longest to shortest wavelength of the photon emitted. Rank from longest to shortest wavelength. To rank items as equivalent, overlap them.
longest to shortest: n = 7 to n = 4 n = 5 to n = 3 n = 3 to n = 2 n = 4 to n = 2
Compare the orbital shown in Parts A and B to the orbital shown here in size, shape, and orientation. Which quantum number(s) would be different for these two orbitals?
mℓ only
Give the numerical value of n corresponding to 2s.
n = 2
Give the numerical value of n corresponding to 3p.
n = 3
Give the numerical value of n corresponding to 4f.
n = 4
Give the numerical value of n corresponding to 5d.
n = 5
Determine the final value of n associated with this emission.
nf = 1
Determine the initial value of n associated with this emission.
ni = 7
For each set of elements represented in this periodic table outline, identify the principal quantum number, n, and the azimuthal quantum number, ℓ, for the highest energy electrons in an atom of one of those elements.
please look at a periodic table for K, Ca: n=4, l=0 for B to Ne: n=2, l=1 for Tl to Rn: n=6, l=1 for Lr (or Rf) to Cn: n=6 l=2 for lanthanides (La to Lu): n=4, l=3
The black line between elements 56 and 71 in the periodic table shown indicates that in the Lanthanide series elements 57 through 70 are listed below the main table, while in the Actinide series elements 89-102 are listed below the main table. Elements 71 and 103 are listed in main table. Identify the outer electron configuration of each element shown in this periodic table outline.
please look at a periodic table Cs: 6s^1 Rf: 7s^2 5f^14 6d^2 Cd: 5s^2 4d^10 Si: 3s^2 3p^2 Xe: 5s^2 4d^10 5p^6 Lv: 7s^2 5f^14 6d^10 7p^4 Lr: 7s^2 5f^14
How would the dx2−y2 orbital in the n=5 shell compare to the dx2−y2 orbital in the n=3 subshell? A. The contour of the orbital would extend further out along the x and y axes. B. The value of ℓ would increase by 2. C. The radial probability function would include two more nodes. D. The orientation of the orbital would be rotated 45∘ along the xy plane. E. The mℓ value would be the same. Drag the appropriate items to their respective bins.
true: A C E false: B D
Classify the following statements as either true or false.
true: The radial probability function shown here and the probability density [ψ(r)]2 both go to zero at the same distance from the nucleus, approximately 1 Å. false: There are two maxima in this function because one electron spends most of its time at an approximate distance of 0.5 Å from the nucleus and the other spends most of its time at an approximate distance of 3 Å from the nucleus. For an s orbital, the number of radial nodes is equal to the principal quantum number, n.
One of the emission lines of the hydrogen atom has a wavelength of 93.07 nm. In what region of the electromagnetic spectrum is this emission found?
ultraviolet region
If so, what color is it?
violet color
Is this line in the visible region of the electromagnetic spectrum?
yes
Calculate the de Broglie wavelength associated with a muon traveling at a velocity of 8.25×105 cm/s
λ = 4.26×10^−10 m
Calculate the wavelength of the radiation released when an electron moves from n= 5 to n=2.
λ = 434 nm
What is the azimuthal quantum number (also called the angular-momentum quantum number), ℓ, for the orbital shown here? Express your answer numerically as an integer.
ℓ= 2